Hydrogen bonds are polar. A hydrogen bond is a type of attractive (dipole-dipole) interaction between an electronegative atom and a hydrogen atom bonded to another electronegative atom. This bond is always formed between a hydrogen atom and a highly electronegative atom like oxygen, nitrogen, or fluorine.
The polarity of hydrogen bonds arises because the hydrogen atom carries a partial positive charge (δ+), while the electronegative atom carries a partial negative charge (δ-). This creates a dipole moment, making the bond polar. The strength of a hydrogen bond is typically between 5 to 30 kJ/mol, which is stronger than van der Waals interactions but weaker than covalent or ionic bonds.
In summary, hydrogen bonds are polar due to the difference in electronegativity between the hydrogen atom and the electronegative atom it is bonded to, resulting in a dipole moment.